Chemistry Objective: Students will: 1. review electron configurations. 2. define valence electrons. 3. identify valence electrons within an electron configuration. Warm-up: Remembering back to electron configurations, how many electrons can each sublevel hold? s holds p holds d holds f holds
Let s review electron configurations real quick. The electron configuration for sodium is: Sodium (Na) 1s 2 2s 2 2p 6 3s 1 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s 7p
Let s review electron configurations real quick. The electron configuration for sodium is: Sodium (Na) 1s 2 2s 2 2p 6 3s 1 # of electrons total # of electrons must equal the atomic number energy level type of orbital 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s 7p
Let s review electron configurations real quick. The electron configuration for sodium is: Sodium (Na) 1s 2 2s 2 2p 6 3s 1 Let s look at Magnesium (Mg) which is right beside sodium. 1s 2 2s 2 2p 6 3s 2 1s 2s 3s 2p 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s 7p
Let s review electron configurations real quick. The electron configuration for sodium is: Sodium (Na) 1s 2 2s 2 2p 6 3s 1 Let s look at Magnesium (Mg) which is right beside sodium. 1s 1s 2 2s 2 2p 6 3s 2 2s 3s 2p 3p 3d Now Aluminum (Al): 1s 2 2s 2 2p 6 3s 2 3p 1 4s 5s 4p 5p 4d 5d 4f 5f 6s 6p 6d 7s 7p
Let s review electron configurations real quick. The electron configuration for sodium is: Sodium (Na) 1s 2 2s 2 2p 6 3s 1 Let s look at Magnesium (Mg) which is right beside sodium. 1s 1s 2 2s 2 2p 6 3s 2 Now Aluminum (Al): 1s 2 2s 2 2p 6 3s 2 3p 1 2s 3s 4s 5s 2p 3p 4p 5p 3d 4d 5d 4f 5f Lastly Silicon (Si): 1s 2 2s 2 2p 6 3s 2 3p 2 6s 7s 6p 7p 6d
Let s review electron configurations real quick. The electron configuration for sodium is: Sodium (Na) 1s 2 2s 2 2p 6 3s 1 Let s look at Magnesium (Mg) which is right beside sodium. Notice Anything? 1s 2 2s 2 2p 6 3s 2 Now Aluminum (Al): 1s 2 2s 2 2p 6 3s 2 3p 1 Lastly Silicon (Si): 1s 2 2s 2 2p 6 3s 2 3p 2
Let s review electron configurations real quick. The electron configuration for sodium is: Sodium (Na) 1s 2 2s 2 2p 6 3s 1 Let s look at Magnesium (Mg) which is right beside sodium. 1s 2 2s 2 2p 6 3s 2 Now Aluminum (Al): 1s 2 2s 2 2p 6 3s 2 3p 1 Lastly Silicon (Si): 1s 2 2s 2 2p 6 3s 2 3p 2 Notice Anything? The number of electrons in the outer most level are increasing by one each time.
Let s review electron configurations real quick. The electron configuration for sodium is: Sodium (Na) 1s 2 2s 2 2p 6 3s 1 Let s look at Magnesium (Mg) which is right beside sodium. 1s 2 2s 2 2p 6 3s 2 Now Aluminum (Al): 1s 2 2s 2 2p 6 3s 2 3p 1 Lastly Silicon (Si): 1s 2 2s 2 2p 6 3s 2 3p 2 Notice Anything? Those electrons are called Valence electrons and they have a trend.
(def) - electrons in the outer most principal energy level of an atom.
(def) - electrons in the outer most principal energy level of an atom. Valence electrons are important because they are the ones that are used in the formation of chemical bonds.
(def) - electrons in the outer most principal energy level of an atom. Valence electrons are important because they are the ones that are used in the formation of chemical bonds. Here is their trend: remains constant Transition Elements can have different numbers of valence electrons. increases by 1
(def) - electrons in the outer most principal energy level of an atom. Valence electrons are important because they are the ones that are used in the formation of chemical bonds. Here is their trend: remains constant 1 2 3 4 5 6 7 8 Transition Elements can have different numbers of valence electrons. increases by 1
Another way of referring to valence electrons are that they are the electrons located in the last s or s and p orbital.
Another way of referring to valence electrons are that they are the electrons located in the last s or s and p orbital. Since the total number of electrons possible in s and p sublevels is eight (8), there can be no more than eight valence electrons in any atom.
Another way of referring to valence electrons are that they are the electrons located in the last s or s and p orbital. Since the total number of electrons possible in s and p sublevels is eight (8), there can be no more than eight valence electrons in any atom. So Sodium has 1 valence electron in its 3s orbital. 1s 2 2s 2 2p 6 3s 1
Another way of referring to valence electrons are that they are the electrons located in the last s or s and p orbital. Since the total number of electrons possible in s and p sublevels is eight (8), there can be no more than eight valence electrons in any atom. So Sodium has 1 valence electron in its 3s orbital. 1s 2 2s 2 2p 6 3s 1 But silicon has 4 valence electrons: 1s 2 2s 2 2p 6 3s 2 3p 2 2 in the 3s and 2 more in the 3p.
Another way of referring to valence electrons are that they are the electrons located in the last s or s and p orbital. Since the total number of electrons possible in s and p sublevels is eight (8), there can be no more than eight valence electrons in any atom. But how many valence electrons would cobalt have? Co: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 7
Another way of referring to valence electrons are that they are the electrons located in the last s or s and p orbital. Since the total number of electrons possible in s and p sublevels is eight (8), there can be no more than eight valence electrons in any atom. But how many valence electrons would cobalt have? Co: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 7 ONLY 2, under these circumstances.
Another way of referring to valence electrons are that they are the electrons located in the last s or s and p orbital. Since the total number of electrons possible in s and p sublevels is eight (8), there can be no more than eight valence electrons in any atom. And arsenic (As) would have As: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 3 5, under these circumstances.
Your Turn: Write the electron configurations for each of the following elements and determine the number of valence electrons. Be sure to circle which electrons would be considered to be valence electrons. Part 1 Part 2 1. fluorine 2. phosphorus 3. calcium 4. iron 5. argon 6. potassium 7. sulfur 8. copper 9. gallium 10. manganese As mentioned transition elements can have varying numbers of valence electrons. In fact copper can have either 2 valence electrons or just 1. Using an orbital diagram, offer an explanation of why copper can have different numbers of valence electrons.